1.
1. a) Write a net ionic equation for the neutralization of NaOH by a component of a buffer
buffer- .5M HC2H302/ .5M NaC2H302 (mixture of both) b) [then] Write a net ionic equaiton for
the neutralization of HCL by a component of the buffer (addition of 3M HCI) c) compare your
results in 2. and 3. Are the base-neutralizing capacity and the acid- neutralizing capacity of the
buffer similar? Explain why or why not. 2. a) Write a net ionic equation for the neutralization of
NaOH (3M) buffer .5M HC2H302 b) compare your results in 2 (above). and 5. Are the base-
neutralizing capacities of bufer and acid comparable? Explain why or why not 3. a)Write a net
ionic equation for the neutralization of HCL (3M) buffer .5M NaC2H302 b) compare your
results in 3. and 6. Are the acid-neutralizing capacities of buffer and salt comparable? Explain
why or why not.
Solution
1. Net ionic equation of buffer,
a) with NaOH
HC2H3O2(aq) + OH-(aq) --> C2H3O2-(aq) + H2O(l)
b) with HCl
C2H3O2-(aq) + H+(aq) --> HC2H3O2(aq)
2. with 3M NaOH,
it neutralizes the acid component of the buffer completely whose concentration in solution = 0.5
M HC2H3O2
3. with 3 M HCl, again the base component of the buffer is completely neutralized with added
acid in solution. The concentration of base component of buffer is = 0.5 M.
Addition of excess base (NaOH) or acid (HCl) destroys the buffer and exceeds the buffer
capacity. The solution is no more a buffer solution.